esti mist titrates 20.0 ml of 0.20 M HBIO with 0.10 M NHOH. Galculate the pH: 1. Before the titration. 2. When the concentration of HBro equal to the concentration of Bro. 3. When number of moles of HBrO are equal to number of moles of bane added Given an acid dissociation constant, K of HBrO-23 x 10.

esti mist titrates 20.0 ml of 0.20 M HBIO with 0.10 M NHOH. Galculate the pH: 1. Before the titration. 2. When the concentration of HBro equal to the concentration of Bro. 3. When number of moles of HBrO are equal to number of moles of bane added Given an acid dissociation constant, K of HBrO-23 x 10.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

13
Please calculate the pH of a buffer solution made up of formic acid and sodium formate. The solution was made by dissolving 0.808 mol of sodium formate, and 0.808 mol of formic acid in 1.80 Liter of water (please assume a total volume for the solution of 1.80 L). (Ka = 1.80 x 10-4) a. pH= 1.93 Ob. pH = 2.11 Oc. pH = 3.08 d. pH = 3.74 QUESTION 2 The Ka for Formic Acid = 1.80 x 10-4. What is the pH of a 0.778 M Formic Acid solution? HA +B+ A + HB+ Oa. pH = 2.11 b. pH = 1.57 c. pH = 1.93 d. pH = 1.81
74. A 25.0-mL sample of 0.125 M pyridine is titrated with 0.100 M HCl. Calculate the pH at each volume of added acid: 0 mL, 10 mL, 20 mL, equivalence point, one-half equivalence point, 40 mL, 50 mL. Sketch the titration curve.
Question 3 Choose the best indicator to use in the titration of a weak base (CH3NH2) methylamine with HCl. Indicator Titration Range Color Change Methyl Orange 3.1 - 4.4 red to orange Oa. Indicator Titration Range Color Change Ob. Methyl red 4.2 -6.3 red to yellow Indicator Titration Range Color Change Oc. Bromothymol blue 6.2 – 7.6 yellow to blue Indicator Titration Range Color Change Od. Thymol blue 8.0 - 9.6 yellow to blue Indicator Titration Range Color Change Oe. Alizarin yellow 10.0 12.0 Colorless to yellow A Moving to the next question prevents changes to this answer. NOV 21 427
answer and explain step by step
1 If you titrate 25.00 mL of 0.05 M NaOH with 0.025 M HCl, a.what is the hydronium ion concentration at the initial stage with no HCl added yet? b.What is the pH of the solution at the start? c. What is the pH of the solution if you add 25 mL of HCl?
4) A buffer solution is made from 135 mL of 0.395 M in HC2H3O2 and 115 mL 0.345 M NaC2H3O2 (the Ka of acetic acid is 1.79 x 10-5). a. Determine the pH of the initial buffer solution. b. What is the buffering range of this solution? c. What is the buffering capacity of this solution? d. What is the maximum volume of 2.00 M HCl solution you can add this buffer before it is no longer effective?
Consider the titration of 100.0 mL of 0.200 M CH3NH2 by 0.100 M HCI. Calculate the pH after 65.0 mL of HCI added. (K for CH3NH2=4.4 × 10-4) A. 10.96 B. 9.75 C. 7.00 D. 3.68 E. 2.54
A solution containing 50.0mL of 0.1800 M NH3 is being titrated with0.3600M HCl. Calculate the pH: i. Initiallyii. After the addition of 12.5 mL of HCliii. After the addition of a total volume of 25.00 mL of HCliv. After the addition of a total volume of 26.00 mL of HCl
20c.
Which of the following will raise the pH of a weak acid HA in aqueous solution? I. addition of HNO3 II. addition of NaCl III. addition of A- with no change in volume IV. titrating with KOH A) || and III B) I and IV C) III and IV D) I and II E) Il and IV
1. calculate the pH of a solution obtained by mixing 30.4 mL of 0.03 M HCL with 31.4 mL of o.1 M HNO3 solution 2.A given weak acid has a pKa of 8.27. Calculate the percent ionized in 0.34 M of the weak acid. 3. Calculate the pH of 0.021 M Sr(OH )2 PLEASE DO ALL THREE